1. Structure & Properties of Matter
Science TAKS Review
Objective 4

2. 7A
Investigate and identify properties of fluids including density, viscosity, and buoyancy

3. Fluids: a substance that can flow and take shape of its container.
Gases – can be compressed
Liquids – diffuse slowly (spread out evenly)

4. The density of steel is the same! Size doesn’t matter! It is a ratio!
steel bar

5. Use the formula sheet – you are given the density and you can read the volume from the cylinder!

6. Ice! Because it is less dense.
Which one floats? Why?
Density of Water: g/mL
Density of Ice: g/mL
Ice! Because it is less dense.

7. The density of water is 1 g/ml
Anything more than that will sink!
The table shows properties of four liquids that are insoluble in water. If the four liquids are poured into an Erlenmeyer flask containing water, which liquid will form a layer below the water?
A Q
B R
C S
D T

8. is the tendency of a less dense substance to float in a
Buoyancy
is the tendency of a less dense
substance to float in a
more dense liquid.
Boats are made so that they have a lower density than water.

9. is the resistance to flow.
Viscosity
is the resistance to flow.
Which is more viscous?
warm syrup or cold syrup?
Cold syrup (high viscosity), because of the strength
of attraction between the particles.

10. REMINDER: Density is a ratio
REMINDER: Density is a ratio! As long as the substance is the same – the density is the same!

12. 7D
Relate the chemical behavior of an element including bonding, to its placement on the periodic table

13. Nonmetals
Metals
Metalloids

14. TRANSITIONMETALS Groups or Family Names Inner earth metals
1) ALKALI METALS
2) ALKALINE METALS
17) HALOGENS
18) NOBLE GASES
TRANSITIONMETALS
Inner earth metals

15. Atoms are Neutral: (#protons = # electrons)
(# protons) Atomic No. 14
Silicon Si
Element Symbol
Atomic Mass
Element Name
Groups/Family (down)
Atoms are Neutral: (#protons = # electrons)
How many protons?
How many electrons? 14
Periods (across) 14

16. A certain atom has a nucleus containing six
protons and eight neutrons and has six
electrons orbiting the nucleus. This atom is a
form of the element —
A silicon
B carbon
C magnesium
D calcium
Elements are identified by the number of protons which = the atomic number!

17. HINT: Same family = similar properties due to same # of valence electrons

18. Number of Valence Electrons
Are electrons in the highest energy level. The noble gases have 8 electrons.
All elements will gain, lose, or share electrons to end up with 8 electrons like the noble gases.
This is called the Octet Rule.

19. Net Ionic Charges Metals will LOSE electrons to form positive ions.
Nonmetals will GAIN electrons to form negative ions.

20. Use your PT
Which of these elements is most likely to donate one electron?
F Be
G Cs
H Rn
J He

21. Noble Gases are inert gases…
Chemical Reactivity
Metals increase in reactivity left and down.
Most reactive metal is?
Nonmetals become more reactive up and to the right.
Most reactive nonmetal is? Fr
Noble Gases are inert gases…
(don’t react easily) F

23. How many atoms do you need?
Atoms will join so the sum of all the charges = zero
O2-
Al3+
O2-
Al3+
O2-
You need 2 Al atoms & 3 O atoms: Al2O3

25. 7E
Classify samples of matter from everyday life as being elements, compounds, or mixtures

26. Has mass and volume (s, l, g)
One type of matter
More than one type of matter physically combined
Uniform throughout (aka. solutions)
Not uniform throughout
Two or more elements chemically combined
One type of atom – cannot be separated

27. Properties of Matter Property – a characteristic
Physical properties:
characteristics that can be observed or measured without changing the identity of the substance.
Ex. Color
Density
Solubility
Melting Point
Chemical properties:
characteristics of a substance’s “ability” to change into a different substance.
Ex. Reactivity
Flammability

30. 8A
Distinguish between physical and chemical changes in matter such as oxidation, digestion, changes in states, and stages in the rock cycle

31. Changes of Matter Physical Changes:
A change that does not produce a new substance.
Usually reversible.
Ex: Ice melts into water.
Chemical Changes:
A change that does produce a new substance.
Usually not reversible.
Ex: Iron rusts forming iron oxide.

32. How do you know a chemical change has occurred?
Physical
change
begins
in the
mouth
Evidence of a
Chemical Change:
Energy (Heat):
absorbed energy (endothermic)
released energy (exothermic)
Gas is produced (bubbles)
Solid (precipitate) forms
Odor or color change occurs
Chemical
change
(Digestion)
occurs
in the
stomach

33. Why are these chemical changes?

34. The Rock Cycle
One of nature’s slowest processes – the rock cycle – is a repeating series of physical and chemical changes in which one type of rock changes to another type.

39. Investigate and identify the law of conservation of mass

40. Law of Conservation of Mass/Matter -Mass is neither created nor destroyed!
The total mass of the substances before they are mixed is equal to the total mass as a mixture.
= 256 g
Zn = 104 g

41. Mass of the reactants = Mass of the products …Always!
1CH4 + 2O2  1CO2 + 2H2O
1 C, 4 H, 4 O = 1 C, 4 H, 4 O
(1x12.0) + (4 x 1.0) + (4x16.0) = (1x12.0) + (4 x 1.0) + (4x16.0)
80 g = 80 g
Ex: How many grams of oxygen react with 16 g of CH4 to create 80 grams of products?
Reactants = Products
x g + 16 g = 80 g
x = 80-16
= 64 g O2

42. Balancing Chemical Equations
CH4 (g) + O2 (g)  CO2 (g) + H2O (g)
Count the number of atoms on both sides
of the arrow.
1 CH4 (g) O2 (g)  1 CO2 (g) H2O (g)
Place a coefficient in front of the compound to
get the same number of atoms in the reactants
and in the products.

43. Guided Practice Ex. 1: Mg + HCl  MgCl2 + H2 Mg + 2 HCl  MgCl2 + H2
Ex. 2: KClO3 − KCl O2
Balanced Equation:
Mg HCl  MgCl2 + H2
Balanced Equation:
2 KClO3 − 2 KCl O2

44. According to the law of conservation of mass, how much zinc was present in the zinc carbonate?
A 40 g
B 88 g
C 104 g
D 256 g

46. In other words: which one is balanced correctly?

47. The chemical equation shows CaCO3 being heated
The chemical equation shows CaCO3 being heated. Which of these statements best describes the mass of the products if 100 g of CaCO3 is heated?
A The difference in the products’ masses is equal to the mass of the CaCO3.
B The sum of the products’ masses is less than the mass of theCaCO3.
C The mass of each product is equal to the mass of the CaCO3.
D The sum of the products’ masses equals the mass of the CaCO3.

48. 9A
Relate the structure of water to its function as the universal solvent

49. Hydrogen and Oxygen covalently bond to each other.
Structure of Water
Polar Molecule:
Hydrogen: Partial positive (+) charge Oxygen: Partial negative () charges.
Hydrogen Bonding
Hydrogen and Oxygen covalently bond to each other.

50. Dissolves so many other substances due to its structure/polarity.
Water as a Universal Solvent
Dissolves so many other substances due to its structure/polarity.
Positive Ion Surrounded by oxygen ()
Negative Ion Surrounded by hydrogen (+)

51. HINT: Any question that asks you about a characteristic of water will have an answer that deals with molecular structure (aka. The formula) including polarity!

54. 9B
Relate the concentration of ions in a solution to physical and chemical properties such as pH, electrolytic behavior, and reactivity

55. Concentrations on Solutions
Solutions can be solids, liquids, or gases.
Unsaturated
Saturated
Supersaturated
More solvent than solute. Ex. Lightly sweetened
Solvent has dissolved all the solute it can hold. Ex. Sweet tea
Solvent holds more solute than is normal. Ex. Rock candy
Dilute: solution made with little solute.
Concentrated: solution made with a lot of solute.

56. Solubility Curves Look at KNO3
Point on the line = Saturated
Point below the line = Unsaturated
Point above the line = Supersaturated

57. Example: Dissolve sugar in hot tea vs. iced tea
Solubility Factors
Temperature & Solids
Solubility increases as the temperature increases for most substances (upward curves)
Example: Dissolve sugar in hot tea vs. iced tea

58. Carbon dioxide gas will go out as the soda warms up making it flat.
Solubility Factors
Temperature & Gases
Solubility of gases in water decreases with increasing temperature.
Example: Soda pop
What happens when you leave a soda out on a hot day?
Carbon dioxide gas will go out as the soda warms up making it flat.
So keep your soda COLD!

59. Pressure & Gases Solubility Factors
Solubility of liquids and solids isn’t affected much.
Gas solubility ALWAYS increases as pressure increases.
The way to get gas to dissolve in liquid is to pressurize the mixture, meaning that the pressure inside a soda can is greater than the pressure outside the can.

63. Electrolytic Behavior
Non-electrolyte: (ex. pure water) No ions present, thus, no electrical conductivity.
Weak electrolyte: (ex.weak acid/base) Few ions present, thus, poor electrical conductivity.
Strong electrolyte: (ex. Strong acid/base)
Salt completely breaks apart to give more ions, conduct more electricity.

64. ____ ___ ____ OH- H+ Acids are: pH less than 7 Sour, like lemons
____ ___ ____
Acids are:
pH less than 7
Sour, like lemons
Change Blue litmus paper to red.
Forms Hydrogen ions
Bases are:
pH more than 7
Bitter and Slippery
Change Red litmus paper will to blue.
Forms Hydroxide ions.
OH- H+

65. Neutralization Reaction:
The pH Scale
Acid
Neutral
Base
Neutralization Reaction:
Acid + Base --> Salt + Water

66. Now You Try!

69. The bonding characteristics of oxygen are
most similar to the bonding characteristics
of —
A hydrogen
B silicon
C helium
D sulfur

70. Know the properties of the groups/families!!

72. Compounds with the same chemical
composition may have different densities because they —
A have differences in reactivity
B are able to bond with oxygen
C vary in solubility
D exist in different phases

78. Which characteristic of water best explains its ability to dissolve a great variety of materials?
A Its transparency in light
B Its electrical conductivity
C Its physical state of matter
D Its molecular arrangement

84. Power plants that discharge warm water into
rivers have a negative effect on aquatic life.
This is because the higher water
temperature —
A increases the pressure of the river water
B increases the pH value of the river water
C decreases sediment solubility in the river
water
D decreases the dissolved oxygen in the
river water

85. Nine groups of students dissolved as much potassium chloride as possible in water. Each group used 100 mL of water heated to a different temperature. Which graph shows the relationship between solubility and temperature for potassium chloride?